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13 Dec 2019

Which of the following statements is false regarding the equilibrium constant, Kc?A) Kc for a reaction at a particular temperature always has the same value.B) Kc for the reverse reaction is the negative of Kc for the forward reaction.C) The numerical value of Kc depends on the form of the balanced equation.D) When quoting Kc it is customary to omit units.

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Jean Keeling
Jean KeelingLv2
17 Dec 2019

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Related questions

1. Consider the following system at equilibrium where delta H° = 18.8 kJ, and Kc = 9.52×10-2, at 350 K.

CH4(g) + CCl4(g) inverse 2CH2Cl2(g)

If the VOLUME of the equilibrium system is suddenly decreased at constant temperature:

The value of Kc A. increases.
B. decreases.
C. remains the same.
The value of Qc A. is greater than Kc.
B. is equal to Kc.
C. is less than Kc.
The reaction must: A. run in the forward direction to reestablish equilibrium.
B. run in the reverse direction to reestablish equilibrium.
C. remain the same. It is already at equilibrium.
The number of moles of CCl4 will: A. increase.
B. decrease.
C. remain the same.

2. Consider the following system at equilibrium where delta H° = -18.8 kJ, and Kc = 10.5, at 350 K.

2CH2Cl2(g) inverse CH4(g) + CCl4(g)

If the VOLUME of the equilibrium system is suddenly increased at constant temperature:

The value of Kc A. increases.
B. decreases.
C. remains the same.
The value of Qc A. is greater than Kc.
B. is equal to Kc.
C. is less than Kc.
The reaction must: A. run in the forward direction to reestablish equilibrium.
B. run in the reverse direction to reestablish equilibrium.
C. remain the same. It is already at equilibrium.
The number of moles of CCl4 will: A. increase.
B. decrease.
C. remain the same.

Consider the following system at equilibrium where H° = -18.8 kJ, and Kc = 10.5, at 350 K.

2CH2Cl2(g) CH4(g) + CCl4(g)

When 0.25 moles of CH4(g) are removed from the equilibrium system at constant temperature:

the value of Kc

A. increases. B. decreases. C. remains the same.

the value of Qc

A. is greater than Kc. B. is equal to Kc. C. is less than Kc.

the reaction must:

A. run in the forward direction to reestablish equilibrium. B. run in the reverse direction to reestablish equilibrium. C. remain the same. It is already at equilibrium.

the concentration of CCl4 will:

A. increase. B. decrease. C. remain the same.

Consider the following system at equilibrium where H° = 111 kJ, and Kc = 6.30, at 723 K:

2NH3(g)--> N2(g) + 3H2(g)

If the TEMPERATURE on the equilibrium system is suddenly decreased:

1- the value of Kc

A. Increases

B. Decreases

C. Remains the same

2- The value of Qc

A. Is greater than Kc

B. Is equal to Kc

C. Is less than Kc

3- The reaction must:

A. Run in the forward direction to reestablish equilibrium.

B. Run in the reverse direction to restablish equilibrium.

C. Remain the same. Already at equilibrium.

4- The concentration of H2 will:

A. Increase.

B. Decrease.

C. Remain the same.

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A. run in the forward direction to reestablish equilibrium.

B. run in the reverse direction to reestablish equilibrium.

C. remain the same. It is already at equilibrium.

4- The number of moles of O2 will:

A. increase.

B. decrease.

C. remain the same.

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